1. Review Chapter 8 & 9: General, Organic, & Biological Chemistry Janice Gorzynski Smith

2. Chapter 8 & 9 Concepts 2  Identify the solvent and solute in a solution  Like dissolves like, predict which molecules will form solutions  Predict the effect of temperature or pressure on a solution  Perform concentration calculations & conversions  Perform dilution calculations  Predict relative changes in colligative properties between multiple solutions  Understand osmotic pressure & how your kidney’s work.  Identify an acid/base reaction, the acid, base, conjugate acid/base  Caculate K a, K b  Use K w to determine concentration of H 3 O + or OH -  Discuss how water acts as both an acid and a base  Perform titration calculations  Communicate how a buffer prevents large pH changes

3. CH 8 Equations & Conversions Molarity = moles of solute (mol) V of solution (L) M 1 V 1 = M 2 V 2

4. CH 9 Equations & Conversions K a = [H 3 O + ][ ] A − [HA] K b = [OH - ][BH + ] [ B] K w = [H 3 O + ][OH − ] = 1.0 x 10 −14 pH = -log[H 3 O + ] Acidic solution: pH 1 x 10 −7 Basic solution: pH > 7  [H 3 O + ] < 1 x 10 −7 Neutral solution: pH = 7  [H 3 O + ] = 1 x 10 −7

5. Solutions, Solubility, & Concentration 1.The solute is the substance present in a lesser amount. 2.The solvent is the substance present in a larger amount. Solubility is the amount of solute that dissolves in a given amount of solvent. REMEMBER: LIKE DISSOLVES LIKE.  In aqueous or liquid phase solutions solubility increases with increasing temperature  Gases dissolved in liquids increase solubility with decreasing temperature and increasing pressure Communicate how much of a solute is dissolved in a solvent using concentration:  % w/v  % v/v  % mass / mass  ppm  Molarity initial valuesfinal values M 1 V 1 = M 2 V 2 Dilution: Adding more solvent to the initial solution. The number of moles solute DOES NOT CHANGE.

6. Colligative Properties Colligative properties are properties of a solution that depend on the concentration of the solute but not its identity.  One mole of any nonvolatile solute raises the boiling point of 1 kg of H 2 O the same amount, 0.51 o C.  One mole of any nonvolatile solute lowers the freezing point of 1 kg of H 2 O by the same amount,1.86 o C. Apply pressure to reverse osmosis. This is how our kidneys filter blood Reverse Osmosis

7. Acids / Bases A Brønsted–Lowry acid is a proton (H + ) donor. A Brønsted–Lowry base is a proton (H + ) acceptor. HA+ B A − HB+B+ + gain of H + acidbaseconjugate base conjugate acid loss of H + HOH H 2 O as a base add H + HOH H + conjugate acid H 2 O as an acid HO − Conjugate base remove H + Strong: Weak: K w = [H 3 O + ][OH − ]

8. Acid / Base Equilibrium & pH H 3 O + (aq) + (aq)HA(g) + H 2 O(l)A − K a = [H 3 O + ][ ] A − [HA] pH = -log[H 3 O + ] OH - (aq) + BH + (aq)B (g) + H 2 O(l) K b = [OH - ][BH + ] [ B] Base dissociation constant acid dissociation constant Low pH (0 ~ 7) [H 3 O + ] high Acidic Conditions High pH (7 ~ 14) [H 3 O + ] low Basic Conditions

9. Common Acid / Base Reactions Neutralization reaction: An acid-base reaction that produces a salt and water. H + (aq) + OH − (aq) H—OH(l) H + (aq) + HCO 3 − (aq) H 2 O(l) + CO 2 (g) H 2 CO 3 (aq) A bicarbonate base, HCO 3 −, reacts with one H + to form carbonic acid, H 2 CO 3. A carbonate base, CO 3 2–, reacts with two H + to form carbonic acid, H 2 CO 3. 2 H + (aq) + CO 3 2– (aq) H 2 O(l) + CO 2 (g) H 2 CO 3 (aq)

10. Titration AH + B  A- + BH + Acid + Base  Conjugate Base + Conjugate Acid Moles of base Moles of base Volume of acid Volume of acid mole–mole conversion factor mole–mole conversion factor M (mol/L) conversion factor M (mol/L) conversion factor Moles of acid Moles of acid Volume of base M (mol/L) conversion factor [1] [2] [3]

11. Buffers [ ] A − [HA] = [H 3 O + ] xKaKa pH of buffer = -log[H 3 O + ] where